Consider the following statements:

(1) If all the reactants are not taken in their stoichiometric ratio. then at least one reactant will be left behind. 

(2) 2 moles of ${\mathrm{H}}_2\left(\mathrm{g}\right)$ and 3 moles of ${\mathrm{O}}_2\left(\mathrm{g}\right)$ produce 2 moles of water

(3) Equal wt. of carbon and oxygen are taken to produce ${\mathrm{CO}}_2$ then $O_2$ is Iimiting reagent (Assume 100% yield in all cases)

The above statements (1), (2), (3) respectively are (T = True, F = False) :

At least one reactant will be left behind if all the reactants are not added in their stoichiometric ratio because if they are not, one of the reactants will function as a limiting agent, causing the reaction to halt.

Due to the fact that H₂ is the limiting reagent, $2{\mathrm{H}}_2+3{\mathrm{O}}_2\to 2{\mathrm{H}}_2\mathrm{O}$ will result.

$\mathrm{C}+{\mathrm{O}}_2\to {\mathrm{CO}}_2$

The molecular weight of oxygen is larger than that of carbon, thus if the weights of carbon and oxygen are removed in equal amounts, oxygen will be left behind. As a result, there will be more moles of carbon than oxygen.